EP2169749B1 - Catalyseur d'électrode pour pile à combustible, procédé servant à produire celui-ci et pile à combustible utilisant le catalyseur d'électrode - Google Patents

Catalyseur d'électrode pour pile à combustible, procédé servant à produire celui-ci et pile à combustible utilisant le catalyseur d'électrode Download PDF

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EP2169749B1
EP2169749B1 EP08777294.3A EP08777294A EP2169749B1 EP 2169749 B1 EP2169749 B1 EP 2169749B1 EP 08777294 A EP08777294 A EP 08777294A EP 2169749 B1 EP2169749 B1 EP 2169749B1
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Prior art keywords
catalyst
metal
fuel cell
cerium
base metal
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EP2169749A4 (fr
EP2169749A1 (fr
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Hiroaki Takahashi
Yosuke Horiuchi
Takahiro Nagata
Tomoaki Terada
Toshiharu Tabata
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Cataler Corp
Toyota Motor Corp
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Cataler Corp
Toyota Motor Corp
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    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J23/00—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00
    • B01J23/002—Mixed oxides other than spinels, e.g. perovskite
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • H01M4/86—Inert electrodes with catalytic activity, e.g. for fuel cells
    • H01M4/90—Selection of catalytic material
    • H01M4/92—Metals of platinum group
    • H01M4/921—Alloys or mixtures with metallic elements
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • H01M4/86—Inert electrodes with catalytic activity, e.g. for fuel cells
    • H01M4/90—Selection of catalytic material
    • H01M4/92—Metals of platinum group
    • H01M4/925—Metals of platinum group supported on carriers, e.g. powder carriers
    • H01M4/926—Metals of platinum group supported on carriers, e.g. powder carriers on carbon or graphite
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M8/00—Fuel cells; Manufacture thereof
    • H01M8/10—Fuel cells with solid electrolytes
    • H01M8/1007—Fuel cells with solid electrolytes with both reactants being gaseous or vaporised
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J23/00—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00
    • B01J23/38—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals
    • B01J23/54—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals combined with metals, oxides or hydroxides provided for in groups B01J23/02 - B01J23/36
    • B01J23/56—Platinum group metals
    • B01J23/63—Platinum group metals with rare earths or actinides
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J23/00—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00
    • B01J23/38—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals
    • B01J23/54—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals combined with metals, oxides or hydroxides provided for in groups B01J23/02 - B01J23/36
    • B01J23/56—Platinum group metals
    • B01J23/64—Platinum group metals with arsenic, antimony, bismuth, vanadium, niobium, tantalum, polonium, chromium, molybdenum, tungsten, manganese, technetium or rhenium
    • B01J23/656—Manganese, technetium or rhenium
    • B01J23/6562—Manganese
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J23/00—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00
    • B01J23/70—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of the iron group metals or copper
    • B01J23/89—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of the iron group metals or copper combined with noble metals
    • B01J23/8933—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of the iron group metals or copper combined with noble metals also combined with metals, or metal oxides or hydroxides provided for in groups B01J23/02 - B01J23/36
    • B01J23/894—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of the iron group metals or copper combined with noble metals also combined with metals, or metal oxides or hydroxides provided for in groups B01J23/02 - B01J23/36 with rare earths or actinides
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J2523/00—Constitutive chemical elements of heterogeneous catalysts
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J35/00—Catalysts, in general, characterised by their form or physical properties
    • B01J35/30—Catalysts, in general, characterised by their form or physical properties characterised by their physical properties
    • B01J35/391—Physical properties of the active metal ingredient
    • B01J35/393—Metal or metal oxide crystallite size
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
    • Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
    • Y02E60/30—Hydrogen technology
    • Y02E60/50—Fuel cells

Definitions

  • the present invention relates to an electrode catalyst for a fuel cell having a high current density and high durability, a method for producing the same, and a fuel cell having such electrode catalyst.
  • a polymer electrolyte fuel cell comprising a pair of electrodes on both sides of a polymer electrolyte membrane that conducts protons produces electromotive force by supplying hydrogen gas as a fuel gas to one of the electrodes (i.e., the fuel electrode: anode), and supplying oxygen gas or air as an oxidant to the other electrode (i.e., the air electrode: cathode).
  • polymer electrolyte fuel cells have been drastically improved by advances such as the following: (1) a polymer electrolyte membrane having high ion conductivity has been developed; and (2) catalyst-carrying carbon coated with an ion-exchange resin (the polymer electrolyte) consisting of a material that is the same as or different from that of the polymer electrolyte membrane is used as the constituent material of the electrode catalyst layer to form what is called a three-dimensional reaction site in the catalyst layer.
  • the polymer electrolyte fuel cell can readily be made smaller and lighter. Due to the characteristics described above, the polymer electrolyte fuel cell is expected to be put in practical use as a power source for mobile vehicles such as electrically powered cars or power sources for small cogeneration systems.
  • the gas diffusion electrode used in a polymer electrolyte fuel cell consists of a catalyst layer, which contains catalyst-carrying carbon materials coated with said ion-exchange resin, and a gas diffusion layer, which not only supplies the reaction gas to the catalyst layer but also collects electrons.
  • the catalyst layer has open areas consisting of micropores formed among secondary or tertiary carbon particles, which are constituents of the catalyst layer, and the open areas function as diffusion channels of the reaction gas.
  • noble metal catalysts such as platinum or platinum alloy, that are stable in ion-exchange resin are generally used.
  • a polymer electrolyte fuel cell involved the use of catalysts comprising a noble metal, such as platinum or platinum alloy, carried on carbon black as cathode and anode catalysts of the electrode catalysts.
  • a noble metal such as platinum or platinum alloy
  • platinum-carrying carbon black is prepared by adding sodium bisulfite to an aqueous solution of platinic chloride, allowing the mixture to react with a hydrogen peroxide solution, preparing the carbon black particles to carry the resulting platinum colloids, washing the resultants, and heat-treating the resultants as needed.
  • Electrodes of a polymer electrolyte fuel cell are prepared by dispersing platinum-carrying carbon black particles in a polymer electrolyte solution to prepare an ink, coating the gas diffusion substrate, such as a carbon paper, with the ink, and drying the substrate.
  • the polymer electrolyte membrane is sandwiched between such two electrodes, followed by a hot press.
  • a membrane electrode assembly (MEA) can be constructed.
  • JP Patent Publication (kokai) No. 2002-289208 (A ) is intended to provide an electrode catalyst for a fuel cell having high durability by inhibiting growth of platinum particles during operation, and discloses an electrode catalyst comprising a conductive carbon material, metal particles carried thereon that are less likely to be oxidized than platinum under acidic conditions, and platinum covering the outer surface of the metal particles.
  • the publication exemplifies an alloy comprising platinum and at least one metal selected from among gold, chromium, iron, nickel, cobalt, titanium, vanadium, copper and manganese as the metal particle.
  • JP Patent Publication (kokai) No. 2002-15744 (A ) is intended to provide a polymer fuel cell that has excellent cathode polarization properties and produces a high cell output, and disclose the catalyst layer of the cathode containing a metal catalyst selected from the group consisting of platinum and platinum alloy and a metal complex containing a given amount of iron or chromium to improve cathode polarization properties.
  • the catalyst layer contains a noble metal catalyst selected from the group consisting of platinum and platinum alloy and a metal complex containing iron or chromium, and the content of the metal complex is 1 to 40 mol% of the combined quantity of the metal complex and the noble metal catalyst.
  • the metal complex containing iron or chromium in the catalyst layer of the cathode can effectively reduce the overvoltage activated by the oxygen reduction reaction of the cathode. Consequently, the cathode polarization properties can be improved, and high cell output can be attained.
  • peroxides are generated in the catalyst layer formed at the interface between a polymer electrolyte membrane and an electrode through a cell reaction, and the generated peroxides are diffused and converted into peroxide radicals, which cause electrolytes to deteriorate.
  • a fuel is oxidized at the fuel electrode, and oxygen is reduced at the oxygen electrode in a fuel cell.
  • an ideal reaction is represented by the following formulae (1) and (2).
  • the hydrogen ions generated at the anode by the reaction represented by formula (1) permeate (diffuse through) the polymer electrolyte membrane in a hydrate state of H + (XH 2 O), and the hydrogen ions that permeate the membrane are then subjected to the reaction represented by formula (2) at the cathode.
  • the electrode reactions at the anode and at the cathode involve the use of the electrode catalyst layer that is in close contact with the polymer electrolyte membrane as the reaction site, and such reactions proceed at the interface between the catalyst in the electrode catalyst layer and the polymer electrolyte membrane.
  • H 2 O 2 hydrogen peroxide
  • a possible mechanism is as follows. That is, hydrogen peroxide can be generated at the hydrogen or oxygen electrode. At the oxygen electrode, for example, hydrogen peroxide is deduced to be generated in a manner represented by the following formula (3) through the incomplete reduction of oxygen. O 2 +2H + 2e - ⁇ 2H 2 O 2 (3)
  • Oxygen that is contained as a contaminant or intentionally included in gas at the hydrogen electrode or oxygen that is dissolved in an electrolyte at the oxygen electrode and diffused through the hydrogen electrode is considered to be associated with the reaction, and such reaction is considered to be represented by a formula identical to said formula (3) or the following formula (4): 2M-H+O 2- ⁇ 2M+H 2 O 2 (4) wherein M is a catalyst metal used for the hydrogen electrode, and M-H is the catalyst metal trapping hydrogen. In general, a noble metal such as platinum (Pt) is used for a catalyst metal.
  • Hydrogen peroxide that is generated on such electrodes separates from the electrodes by diffusion or other means and migrates into an electrolyte.
  • Hydrogen peroxide is a substance having a potent oxidizing power and oxidizes many types of organic matter that constitute an electrolyte.
  • the detailed mechanism thereof has not been elucidated, it is often considered that hydrogen peroxide produces hydroxyl radicals, and such hydroxyl radicals function as direct reactants for oxidization.
  • the radicals generated by the reaction by such as following formula are considered to abstract hydrogen from the organic matter of an electrolyte or cleave another bond.
  • the cause for radical generation has not yet been elucidated; however, contact with a heavy-metal ion is considered to result in catalyst activity. Further, radical generation is considered to be caused by heat, light, or the like.
  • JP Patent Publication (kokai) No. 2001-118591 (A ) discloses a technique to solve the abovementioned problem, wherein the technique can prevent deterioration of a fuel cell caused by radicals by adding a compound, which "degrades,” “inactivates” and “traps and inactivates” radicals generated by permeated hydrogen, to the electrolyte. More specifically, transition metal oxides, such as manganese oxides, ruthenium oxides, cobalt oxides, nickel oxides, chromium oxides, iridium oxides or lead oxides, which catalytically degrade peroxides, are dispersed and incorporated into a polymer electrolyte.
  • transition metal oxides such as manganese oxides, ruthenium oxides, cobalt oxides, nickel oxides, chromium oxides, iridium oxides or lead oxides, which catalytically degrade peroxides, are dispersed and incorporated into a polymer electrolyte
  • a stabilizer for peroxide such as a tin compound, that inhibits generation of peroxide radicals may be dispersedly incorporated therein.
  • a compound having a phenolic hydroxyl group that traps and inactivates the generated peroxide radicals may be incorporated.
  • JP Patent Publication (kokai) No. 2002-15744 (A ) discloses, when a metal complex having iron or chromium is used as a promoter , a high cell output can be attained at the initial stage.
  • iron or chromium is eluted during the use of a fuel cell, and it disadvantageously causes the durability of a fuel cell to deteriorate as a contaminant of an electrolyte.
  • JP Patent Publication (kokai) No. 2001-118591 (A ) comprising an addition of a compound that "degrades,” “inactivates” and “traps and inactivates” radicals, peroxides are not sufficiently suppressed, and further technical development is needed to improve fuel cell durability.
  • JP Patent Publication (kokai) No. 2006-236927 (A ) discloses the invention in which a membrane electrode junction for a solid polymer fuel cell having high power generation performance and capable of generating power stably for a long time contains a catalyst comprising an alloy of platinum and at least one metal selected from among cerium and manganese on a carbon carrier in the catalyst layer of either an anode or cathode.
  • this publication discloses a Pt/Ce catalyst and a Pt/Mn catalyst.
  • JP Patent Publication (kokai) No. 2006-102568 (A ) discloses a Pt/M catalyst (wherein M represents at least one member selected from a group consisting of a transition metal element, element III and rare-earth element, such as Fe, Ni, Co, Cr, Mn, Ti, Ag, Ce, La, Y and Al).
  • JP Patent Publication (kokai) No. S-61-8851 (A) (1986 ) discloses a Pt/Cr-Ce alloy catalyst.
  • the catalysts such as Pt/Ce catalyst, the Pt/Mn catalyst, the Pt/M catalyst and the Pt/Cr-Ce alloy catalyst disclosed in JP Patent Publication (kokai) No. 2006-236927 (A ), JP Patent Publication (kokai) No. 2006-102568 (A ) and JP Patent Publication (kokai) No. S-61-8851 (A) (1986 ) did not perform satisfactorily in terms of high current density and high durability.
  • US5079107 describes a ternary catalyst containing platinum, chromium and cerium.
  • the present invention provides a fuel cell with improved durability, and in particular, with the improved capacity for power generation in a high current density region.
  • the present invention also provides a method for producing an electrode catalyst for a fuel cell and a fuel cell with improved durability and capacity for power generation in a high current density region using said electrode catalyst for a fuel cell as a cathode catalyst and/or anode catalyst.
  • the present inventor found that the abovementioned problems could be resolved with the use of an alloy having a specific composition as a catalyst metal particle, thereby completing the present invention.
  • the first aspect of the present invention relates to an electrode catalyst for a fuel cell comprising catalyst metal particles of a noble metal-base metal-Ce (cerium) ternary alloy carried on carbon materials.
  • the noble metal is at least one member selected from among Pt, Ru, Rh, Pd, Ag and Au
  • the base metal is at least one member selected from among Ir, Co, Fe, Niand Mn
  • the relative proportion (i.e., the molar proportion) of noble metal:base metal:Ce (cerium) is 20 to 95:5 to 60:0.1 to 3.
  • a particularly preferable example is a Pt-Fe-Ce ternary alloy in which the noble metal is platinum (Pt) and the base metal is iron (Fe).
  • the average particle diameter of the catalyst metal particles carried on carbon materials is preferably 3 to 20 nm, and more preferably 5 to 10 nm.
  • the second aspect of the present invention relates to a method for producing an electrode catalyst for a fuel cell consisting of catalyst metal particles of a noble metal-base metal-Ce (cerium) ternary alloy carried on carbon materials, wherein the noble metal is at least one member selected from among Pt, Ru, Rh, Pd, Ag and Au, the base metal is at least one member selected from among Ir, Co, Fe, Ni and Mn, and the relative proportion (i.e., the molar proportion) of noble metal:base metal:Ce (cerium) is 20 to 95:5 to 60:0.1 to 3, and preferably 40 to 80:15 to 40:0.1 to 3.
  • the noble metal is at least one member selected from among Pt, Ru, Rh, Pd, Ag and Au
  • the base metal is at least one member selected from among Ir, Co, Fe, Ni and Mn
  • the relative proportion (i.e., the molar proportion) of noble metal:base metal:Ce (cerium) is 20 to 95:5 to 60:0.1 to 3, and preferably 40
  • the method comprises steps of adding a noble metal salt, a base metal salt and a Ce (cerium) salt to a water dispersion of the carbon materials, hydroxylating the noble metal salt, the base metal salt and the Ce (cerium) salt under alkaline conditions, reducing the noble metal hydroxide, the base metal hydroxide and the Ce (cerium) hydroxide, and alloying the reduced noble metal, base metal and Ce (cerium).
  • the noble metal be platinum (Pt)
  • the base metal be iridium (Ir) and/or cobalt (Co)
  • the average particle diameter of the catalyst metal particles be 3 to 20 nm, with 5 to 10 nm being more preferable, as described above.
  • the third aspect of the present invention relates to a polymer electrolyte fuel cell using the above electrode catalyst as a cathode catalyst and/or anode catalyst.
  • the polymer electrolyte fuel cell of the present invention involves the use of an electrode catalyst that satisfies conditions regarding high catalytic activity and excellent durability. Accordingly, the polymer electrolyte fuel cell of the present invention is excellent in terms of durability and the capacity for power generation.
  • a noble metal-base metal-Ce (cerium) ternary alloy is used for catalyst metal particles. This can remarkably improve the capacity for power generation in a high current density region and durability of a fuel cell.
  • the present invention involves alloying of Pt, a base metal and Ce, the effects of the addition of Ce can be maintained. Also, the ternary alloy can improve - activity and provide effects of inhibiting alloy disintegration, compared with a case in which Ce alone is added. This can provide a catalyst satisfying conditions regarding initial performance and durability.
  • the base metal which is the third element to be added (except for Pt and Ce) having excellent catalytic activity, is not particularly limited. Ir and Co exhibit particularly high activity.
  • a catalyst of Pt/base metal (preferably Ir and/or Co)/Ce alloy can remarkably extend the durability life of the polymer electrolyte fuel cell.
  • Fig. 1 shows the correlation between cell voltage and the endurance time of a fuel cell using catalysts selected in examples and comparative examples.
  • a base metal and Ce When platinum, a base metal and Ce are alloyed, halides such as chlorides and bromides, alkoxides such as methoxide and ethoxide, oxides, nitrates, and sulfides of each of platinum, a base metal and Ce can be extensively used as starting compounds comprising platinum, a base metal and Ce. Alloying can be preferably carried out by subjecting the reduced platinum component, base metal component and Ce component to heat treatment at 600 to 900°C under an inert gas atmosphere.
  • Particle diameters of an alloy catalyst of platinum, a base metal and Ce are preferably 3 to 20 nm in order to realize high activity. If the particle diameter is smaller than 3 nm, particles easily induce aggregation or dissolution/reprecipitation, thereby particle size increases. If the particle diameter is greater than 20 nm, the surface area would be relatively small in relation to the amounts of alloy metal catalysts to be used. Thus, sufficient catalytic activity cannot be realized. In this respect, particle diameters of an alloy catalyst of platinum, a base metal and Ce are more preferably 3 to 15 nm.
  • CMOS complementary metal-oxide-semiconductor
  • CMOS complementary metal-oxide-semiconductor
  • CMOS complementary metal-oxide-semiconductor
  • activated carbon a carbon-semiconductor
  • a fluorine polymer electrolyte is a fluorine polymer compound with an electrolyte group, such as a sulfonic acid group or carboxylic acid group.
  • a fluorine polymer electrolyte used for the fuel cell of the present invention is a polymer comprising a fluorocarbon or hydrofluorocarbon framework with an electrolyte group, such as a sulfonic acid group. It may comprise within its molecules an ether group, chlorine, a carboxylic acid group, a phosphoric acid group or an aromatic ring.
  • a polymer having perfluorocarbon as a main chain with the sulfonic acid group through a spacer such as perfluoro ether and an aromatic ring is used.
  • a spacer such as perfluoro ether and an aromatic ring
  • a hydrocarbon polymer electrolyte used for the fuel cell of the present invention comprises a hydrocarbon portion in any positions of a molecular chain constituting a polymer compound with an electrolyte group.
  • electrolyte groups include a sulfonic acid group and a carboxylic acid group.
  • the loading density of platinum was 35% by weight
  • the loading density of iridium was 12% by weight
  • the loading density of cerium was 0.5% by weight.
  • the XRD was measured, only the peak of Pt was observed, and the formation of a solid solution of the added elements was confirmed from the peak shift in the (111) plane of Pt in the direction of high angle side at around 39°C.
  • the peaks of Pt, Ir and Ce were observed in the particles.
  • the lattice constant of Pt determined from the peak position in the (111) plane of Pt via XRD was 3.906 ⁇
  • the Pt particle diameter determined based on the half value was 5.5 nm.
  • carbon powder having a high specific surface area was added to 0.5L of pure water and dispersed therein.
  • a hexahydroxo platinum nitrate solution including 4.5g of platinum, a cobalt nitrate solution including 0.5g of cobalt and cerium nitrate including 0.05g of cerium were added dropwise in such order, and were then thoroughly blended with the carbon.
  • 0.1N ammonia (about 100mL) was added thereto in order to bring the pH level to 10, thereby forming the respective hydroxides to precipitate them on the carbon.
  • the dispersion was filtered, and the resulting powder was vacuum-dried at 100°C for 10 hours.
  • the resultant was kept at 400°C for 2 hours in hydrogen gas and subjected to a reducing treatment, and the resultant was then kept at 800°C for 10 hours in nitrogen gas to alloy it.
  • the catalyst was agitated in 1L of a 2 mol/L nitric acid solution, and the resultant was kept in a liquid at 60°C for 1 hour, followed by filtering. The resulting cake was vacuum-dried at 100°C for 10 hours to obtain catalyst powder.
  • the loading density of platinum was 43% by weight
  • the loading density of cobalt was 3% by weight
  • the loading density of cerium was 0.5% by weight.
  • the XRD was measured, only the peak of Pt was observed, and the formation of a solid solution of the added elements was confirmed from the peak shift in the (111) plane of Pt in the direction of high angle side at around 39°C.
  • the peaks of Pt, Co and Ce were observed in the particles.
  • the lattice constant of Pt determined from the peak position in the (111) plane of Pt via XRD was 3.906 ⁇
  • the Pt particle diameter determined based on the half value was 5.9nm.
  • PtFeCe was synthesized according to the method of Example 1, using iron nitrate instead of the iridium nitrate solution.
  • PtNiCe was synthesized according to the method of Example 1, using nickel nitrate instead of the iridium nitrate solution.
  • PtMnCe was synthesized according to the method of Example 1, using manganese nitrate was used instead of the iridium nitrate solution.
  • the loading density of platinum was 35% by weight and the loading density of iridium was 12% by weight.
  • the lattice constant of Pt determined from the peak position in the (111) plane of Pt was 3.902 ⁇ , and the Pt particle diameter determined based on the half value was 5.4nm.
  • the catalyst powder (10.0g) of Comparative Example 1 was added to 0.5L of pure water and dispersed therein. Cerium nitrate including 0.05g of cerium was added dropwise thereto and was then thoroughly blended with the carbon. 0.1N ammonia (about 100mL) was added thereto in order to bring the pH level to 10, thereby forming the respective hydroxides to precipitate them on the carbon. The dispersion was filtered, and the resulting powder was dried in the air at 100°C for 15 hours.
  • the catalyst was agitated in 1L of a 2 mol/L nitric acid solution, and the resultant was kept in a liquid at 60°C for 1 hour, followed by filtering. The resulting cake was vacuum-dried at 100°C for 10 hours to obtain catalyst powder.
  • the loading density of platinum was 43% by weight and the loading density of cobalt was 3% by weight.
  • the lattice constant of Pt determined from the peak position in the (111) plane of Pt was 3.846A, and the Pt particle diameter determined based on the half value was 5.6nm.
  • Cerium nitrate was added dropwise to the catalyst powder of Comparative Example 3 to obtain PtCo+Ce.
  • PtFe was obtained according to the method of Comparative Example 1, using iron nitrate instead of iridium nitrate.
  • Cerium nitrate was added dropwise to the catalyst powder of Comparative Example 5 to obtain PtFe+Ce.
  • PtNi was obtained according to the method of Comparative Example 1, using nickel nitrate instead of iridium nitrate.
  • Cerium nitrate was added dropwise to the catalyst powder of Comparative Example 7 to obtain PtNi+Ce.
  • PtMn was obtained according to the method of Comparative Example 1, using manganese nitrate instead of iridium nitrate.
  • Cerium nitrate was added dropwise to the catalyst powder of Comparative Example 9 to obtain PtMn+Ce.
  • the initial voltage was measured. Characteristics of the current-voltage were measured by setting the unit cell temperature at 80°C and supplying a humidified air, which had been passed through a bubbler heated at 60°C, to the cathode electrode with a stoichiometric ratio of 3 and humidified hydrogen, which had been passed through a bubbler heated at 60°C, to the anode electrode with a stoichiometric ratio of 3. Catalyst performances were compared by continuing the measurement until their current-voltage was stable and then comparing the results of measurement at the current density of 0.1 A/cm 2 . The amount of Pt at each electrode was 0.3 mg/cm 2 .
  • the unit cell temperature was set at 80°C, a humidified air, which had been passed through a bubbler heated at 60°C, was supplied to the cathode electrode with a stoichiometric ratio of 3, and humidified hydrogen, which had been passed through a bubbler heated at 60°C, was supplied to the anode electrode with a stoichiometric ratio of 3.
  • the current values were varied from 0 CV ⁇ 0.1 A/cm 2 every 5 seconds.
  • the voltage values at 0.1A/cm 2 were plotted and durability was compared.
  • Example 1 Catalyst properties and cell properties of Examples 1 to 5 and Comparative Examples 1 to 10 are summarized in Table 1. Further, properties and durability of the cells of Examples 1 and 2 and Comparative Examples 1, 2, and 3 are shown in Fig. 1 .
  • Table 1 Sample Catalyst particle diameter (nm) Loading density (%) Cell performance @0.1A/cm 2 (V) Pt M (third element) Ce Initial After durability test (after 30,000 hrs)
  • Example 1 PTIrCe 5.5 35.0 12.0 0.5 763 746
  • Example 2 PtCoCe 5.9 43.0 3.0 0.5 775 740
  • Example 3 PtFeCe 6.1 45.5 4.6 0.5 788 772
  • Example 4 PtNiCe 5.7 44.2 3.4 0.5 768 736
  • Example 5 PtMnCe 6.0 47.6 2.9 0.5 778 741 Comparative Example 1 PtIr 5.4 35.0 12.0 - 733 676 Comparative Example 2 PtIr+Ce
  • the PtCo catalyst (Comparative Example 3) was found to show a lowered voltage after the durability test. This is considered to result from lowered catalyst activity due to separation of a Co solid solution and deterioration of an electrolyte membrane due to elusion of Co into the membrane.
  • the state of the PtCo catalyst in the catalyst layer after the durability test was actually verified by XRD, the lattice constant was found to be increased due to Co elution, compared with the lattice constant at the initial stage.
  • the catalyst consisting of only PtIr did not show significant separation of an Ir solid solution, although lowering of the voltage was observed. This is considered to result from deterioration of an electrolyte membrane caused by hydrogen peroxide generated during the durability test.
  • a catalyst that additionally comprises Ce does not show significant lowering in the voltage as a result of the addition of Ce (i.e., hydrogen peroxide degradation), catalyst activity is low, and satisfactory performance cannot be attained.
  • ternary alloy in Examples 1 and 2 was found to yield improved voltage and durability. It would appear that these significant effects were caused by the improved catalyst activity and durability of the ternary alloys.
  • the inhibiting effects of deterioration of an electrolyte membrane caused by degradation of hydrogen peroxide obtained by alloying Ce and the inhibiting effects of separation of an alloy solid solution caused by preparing a ternary alloy are characteristics of the catalyst of the present invention.
  • the initial state and the state after the durability test of the catalysts of Examples 1 and 2 in the catalyst layer were compared by XRD. As a result, the lattice constant did not substantially change, and separation of an alloy solid solution was not observed.
  • Example 1 showed higher alloy stability due to the effects of Ir addition.
  • the catalyst of Example 1 can be regarded as a catalyst with high durability.
  • Examples 3 to 5 show catalyst performances of ternary alloys prepared with the use of Fe, Ni, or Mn as a base metal instead of Ir or Ce. As in the case of Examples 1 and 2, these ternary alloys show improved initial performance and durability. Comparative Examples 5, 7 and 9 show the initial performance and durability of each element in terms of the binary system. Comparative Examples 4, 6, 8 and 10 show the initial performance and durability of each element in terms of the binary system and the system with the addition of Ce. In Comparative Examples 5, 7 and 9, lowered performance (i.e., lowered voltage) after the durability test was observed due to the lack of Ce addition. Further, Comparative Examples 4, 6, 8 and 10 show insufficient catalyst activity caused by unalloying of Ce.
  • Fe was known to have had high catalyst activity and high initial performance; however, it could not attain satisfactory durability due to the accelerated deterioration of an electrolyte and lowered performance.
  • Such drawbacks could be overcome with the additioni of Pt, Fe, and Ce to prepare ternary alloys.
  • the PtFeCe catalyst has high durability and excellent activity.
  • the present invention provides a catalyst having both initial performance and durability by having the effects of the improved activity and inhibition of alloy disintegration realized by the preparation of ternary alloys of Pt, a base metal and Ce.
  • the present invention contributes to practical applications and spreading of fuel cells.

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  • Electrochemistry (AREA)
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  • Manufacturing & Machinery (AREA)
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Claims (7)

  1. Catalyseur d'électrode pour pile à combustible comprenant des particules métalliques de catalyseur à base d'un alliage ternaire métal noble-métal de base-Ce (cérium) supportées sur des matériaux carbonés, dans lequel le métal noble est au moins un élément choisi parmi Pt, Ru, Rh, Pd, Ag et Au, le métal de base est au moins un élément choisi parmi Ir, Co, Fe, Ni et Mn, et la proportion molaire relative métal noble:métal de base:Ce (cérium) est de 20 à 95:5 à 60:0,1 à 3.
  2. Catalyseur d'électrode pour pile à combustible selon la revendication 1, dans lequel le métal noble est le platine (Pt) et le métal de base est le fer (Fe).
  3. Catalyseur d'électrode pour pile à combustible selon la revendication 1 ou 2, dans lequel le diamètre de particules moyen des particules métalliques de catalyseur est de 3 à 20 nm.
  4. Procédé de production d'un catalyseur d'électrode pour pile à combustible, dans lequel les particules métalliques de catalyseur constituées d'un alliage ternaire métal noble-métal de base-Ce (cérium) sont supportées sur des matériaux carbonés, le métal noble est au moins un élément choisi parmi Pt, Ru, Rh, Pd, Ag et Au, le métal de base est au moins un élément choisi parmi Ir, Co, Fe, Ni et Mn, et la proportion molaire relative métal noble:métal de base:Ce (cérium) est de 20 à 95:5 à 60:0,1 à 3,
    le procédé comprenant les étapes d'ajout d'un sel de métal noble, d'un sel de métal de base et d'un sel de Ce (cérium) à une dispersion aqueuse de matériaux carbonés, d'hydroxylation du sel de métal noble, du sel de métal de base et du sel de Ce (cérium) dans des conditions alcalines, de réduction de l'hydroxyde de métal noble, de l'hydroxyde de métal de base et de l'hydroxyde de Ce (cérium), et de formation d'un alliage à base de l'hydroxyde de métal noble, de l'hydroxyde de métal de base et de l'hydroxyde de Ce (cérium) réduits.
  5. Procédé de production d'un catalyseur d'électrode pour pile à combustible selon la revendication 4, dans lequel le métal noble est le platine (Pt), et le métal de base est l'iridium (Ir) et/ou le cobalt (Co).
  6. Procédé de production d'un catalyseur d'électrode pour pile à combustible selon la revendication 4 ou 5, dans lequel le diamètre de particules moyen des particules métalliques de catalyseur est de 3 à 20 nm.
  7. Pile à combustible à électrolyte polymère comprenant le catalyseur d'électrode selon l'une quelconque des revendications 1 à 3 à titre de catalyseur de cathode et/ou de catalyseur d'anode.
EP08777294.3A 2007-06-11 2008-06-11 Catalyseur d'électrode pour pile à combustible, procédé servant à produire celui-ci et pile à combustible utilisant le catalyseur d'électrode Not-in-force EP2169749B1 (fr)

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PCT/JP2008/061073 WO2008153189A1 (fr) 2007-06-11 2008-06-11 Catalyseur d'électrode pour pile à combustible, procédé servant à produire celui-ci et pile à combustible utilisant le catalyseur d'électrode

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EP2169749A4 (fr) 2011-11-02
EP2169749A1 (fr) 2010-03-31
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US8338051B2 (en) 2012-12-25

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